In general, it is observed that the rate of a chemical reaction doubles with every 10° rise in temperature. If this generalisation holds for a reaction in the temperature range 298 K to 308 K, what would be the value of activation energy for this reaction ? (R` = 8.314 JK^(-1) mol^(-1)`)

Explanation

To find the activation energy (Ea) for the reaction, we can use the Arrhenius equation and the information provided in the question. The general observation is that the rate of a chemical reaction doubles with every 10°C rise in temperature.

### Step-by-Step Solution:

1. **Identify the given data:**
- Initial temperature (T1) = 298 K
- Final temperature (T2) = 308 K
- The rate doubles when the temperature increases by 10°C (or 10 K).
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